A monatomic ideal gas expands in a reversible adiabatic process. The initial temperature of the gas amounts to T; and the mole number is equal to n. The final temperature T; = T/4. Calculate the work done by the gas? O a. -5/8 nRT; O b. -9/8 nRT; O c. 3/2 nRT; O d. 5/2 nRT; O e. 9/8 nRT
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- 2.0 mol of CO2 gas (assumed to be a perfect gas with Cv,m = 28.8 JK-1mol-1) is in a cylinder with a massless piston of cross-section 100 cm2 at 10°C and 9.0 atm. The gas expands adiabatically against an external pressure of 1.5 atm until the piston moves 15 cm. Calculate (a) q; (b) w; (c) ΔU; (d) ΔT; (e) ΔS for this process.Q1) A constant volume tank contain 1 mole ofC7H14and 12 mole of O2 gas at a temperature of 25 °C and 1 bar. The contents of the tank is ignited and C7H14 is burned completely and final products temperature is found to be 1700 K. Determine the heat transfer during this process. ( take daltaHo = -47800 kJ/kg).A piston/cylinder setup contains 1 kg of air at 20°C with an initial volume of V1=0.1 m3, as shown in Fig. Q7. Initially, the piston rests on some stops, but it is possible for it to move within the cylinder without friction. To lift the piston and start such motion, an air pressure of 1400 kPa is required. Now, heat is transferred to the system so that the temperature of the air reaches to a final value of 300°C. Fig. Q7 A. Which statement is true? The air can lift the piston before the temperature reaches to 300°C The air cannot lift the piston before the temperature reaches to 300°C
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- Consider one mole of a simple ideal gas enclosed in a cylindrical piston with rigid impermeable adiabatic walls. The piston has a cross sectional area ofA = 0.10 m^2 and the cylinder enclosing the gas has a height of h = 1.0 cm. The gas inside the piston has a temperature T = 300.K. Recall that the internal energy for an ideal gas is U= n cV,mT, where cV,m= 1.5 R is the molar heat capacity for the ideal gas. mass m = 15.3E3kg is placed on the top of the piston, but that the piston top remains rigid. The external pressure applied is 1.5E6 Pa. The equilubrium volume for the gas is 1.6E-3 m^3. Suppose that the piston is now allowed to move within the cylinder, but that the walls remain adiabatic and impermeable so that no heat flows into the gas. The gas system will ultimately move to a new equilibrium state. We will now characterize the final equilibrium state and the changes resulting from the process. Define the (Total System) = (the gas enclosed in the cylinder) plus (the mass placed…1. Air enters a machine at 373°K with a speed of 200 m/s and leaves it at 293°C. If the flow is adiabatic, and the work output by the machine is 105 N · m/kg, what is the exit air speed? What is the exit speed when the machine is delivering no work? 2. Two jets of air with the same mass flow rate mix thoroughly before entering a large closed tank. One jet is at 400◦K with a speed of 100 m/s and the other is at 200°K with a speed of 300 m/s. If no heat is added to the air, and there is no work done, what is the temperature of the air in the tank?A monatomic ideal gas with volume 0.150 L is rapidly compressed, so the process can be considered adiabatic. If the gas is initially at 1.01 105 Pa and 3.00 102 K and the final temperature is 481 K, find the work done by the gas on the environment, Wenv.Wenv =
- Q1) A constant volume tank contain 1 mole of C,H14 and 12 mole of O2 gas at a temperature of 25 °C and 1 bar. The contents of the tank is ignited and C8H18is burned completely and final products temperature is found to be 1700 K. Determine the heat transfer during this process. ( take AHo = -47800 kJ/kg).A piston/cylinder arrangement contains one mole of an ideal gas (the system) initially at 10.0 atm pressure and 300 K, as shown in the accompanying illustration. Neglecting the mass of the piston, neglecting friction, and assuming isothermal conditions throughout, the pin restraining the piston is removed. For the resulting process: (g = 9.807 m sR7) (a) What is qsyst if the mass of the weight is zero? (b) What is qsyst if the mass of the weight is 100 kg? (c) What is qsyst if the mass of the weight is 1017.4 kg?One mole of nitrogen (N2) is cooled from an initial temperature and pressure of 700 K and 10 bar to a final temperature of 300 K. The heat capacity of nitrogen may be taken as: Cp,m = 28.58 + 3.77 × 10-3 T where Cp,m is in J mol-1 K-1 and T is in Kelvin. Assuming nitrogen behaves as an ideal gas, calculate q, w, ∆U, and ∆H for this process when it is carried out (a) at constant pressure, and (b) at constant volume. Compare the values obtained for the two cases.